Solution Chemistry Simplified Based on Arrhenius' Theory of Electrolytic Dissociation and Hydration for All Concentrations Collected Research Work, Dedicated to Svante August Arrhenius (1859 – 1927).

Arrhenius theory of partial dissociation of electrolytes rose to its heights and fame when he was awarded the Nobel Prize (1903). While the theory was still being developed to account for the non-ideal properties of electrolytes at higher concentrations, it was unfortunately replaced by Lewis’ empirical concepts of activity and activity coefficients. With the near success of the Debye-Huckel theory of inter-ionic interactions for very dilutions, the latter was erroneously extended over the next few decades by extended parametrical equations to higher concentrations assuming complete dissociation at all concentrations. This eventually turned solution theory into a mere catalogue of parameters. Therefore, the present author abandoned it all and started systematically analyzing the available experimental data as such. She found that with the degrees of dissociation and ‘surface’ and ‘bulk’ hydration numbers obtained from vapor pressure data, properties of electrolytes could be explained quantitatively over the whole concentration range, using simple mathematical equations.

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